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2 marksEnergetics

CAPE Chemistry Unit 1 · 2007 · Paper 2 · Question 1(b)(ii)

A student carries out an experiment to determine the enthalpy change of the reaction between magnesium and hydrochloric acid. She measures the steady temperature of 100 cm³ of hydrochloric acid in a polystyrene cup. She then places a 10 cm long piece of magnesium, of mass 0.5971 g, in the acid and records the temperature every 30 seconds for 4 minutes, while stirring at regular intervals.

Given that the initial and final temperatures are 28°C and 57°C respectively, sketch a typical graph for the results of the experiment to illustrate how the student arrived at the temperature change, ΔT, for the experiment.

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Other parts of this question

  1. 1(a)Use Hess's law to calculate the enthalpy change for the following reaction: 2Mg (s) + O2(g) → 2MgO(s)[3 marks]
  2. 1(b)(i)Explain the reason for stirring the mixture at regular intervals.[1 mark]
  3. 1(b)(iii)Give the main source of error for the experiment.[1 mark]
  4. 1(b)(iv)Calculate the enthalpy change, in kJ mol⁻¹ of Mg for the reaction at constant pressure, given ΔT = 29.0°C, C = 4.20 Jg⁻¹ °C⁻¹. The density of dilute HCl is…[3 marks]
  5. 1(c)(i)Use the results of your calculation in (b)(iv) above to state whether the reaction is endothermic or exothermic.[1 mark]
  6. 1(c)(ii)Draw a clearly labelled energy profile diagram for the reaction between magnesium and hydrochloric acid. Include on your diagram the enthalpy change for the…[4 marks]

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